SYMBOLS, FORMULAS AND MOLAR MASSES OBJECTIVES 1. To correctly write and interpret chemical formulas 2. To calculate molecular weights from chemical formulas 3. To calculate moles from grams using chemical formulas INTRODUCTION Part I. Symbols and formulas An element is a homogeneous pure substance made up of identical atoms. All matter is made up of elements and, since chemistry is the study of matter, it is convenient to use symbols to represent the elements rather than using the entire name. By international agreement, specific symbols are assigned to each element (Note: This means that while names of the elements vary with language, symbols are constant throughout the world.) Each element is assigned a one- or two-letter symbol. The first letter is capitalized, the second (if there is one) is not. While this often seems trivial, it is in fact a very important point. For example, in chemical language Co represents cobalt, which is a metal and an element, while CO represents carbon monoxide, a compound which is a colorless, odorless gas! Even when there is not an obvious correspondence, for instance "MN", it can cause confusion. Do you mean the element manganese? Did you forget a letter and mean something else? Are you using "M" to represent something else entirely? Chemists sometimes use "M" to represent any metal. It is well worth the trouble to memorize the symbols for common elements. Since compounds consist of elements, the chemical formulas of compounds also consist of elements with subscripts used to denote the number of atoms per molecule. If there is no subscript, it is implied that there is one of that kind of atom. Ones never appear in chemical formulas. Not only do subscripts denote ratios of atoms, they also denote the ratio of moles of element to one mole of compound. Parentheses can be used to show groups of atoms, with the subscripts showing how many groups there are. Parentheses are not used if there is only one group. Examples: For one mole of the following compounds, how many moles of each element are present? MgCl2 1 mole Mg, 2 moles Cl Mg(NO3)2 1 mole Mg, 2 moles N, 6 moles O NaNO3 1 mole Na, 1 mole N, 3 mole O AgCl 1 mole Ag, 1 mole Cl Part II. Molar Masses Each atom has a different size and therefore a different mass. The relative masses of each element can be found on the periodic table. For example, one atom of magnesium weighs 24.31 amu (atomic mass units). However, one mole of magnesium weighs 24.31 g. (Moles were planned that way!) Since one mole of MgCl2 consists of one mole of magnesium and two moles of chlorine, the mass of one mole of MgCl2 must be the sum of the masses of the elements. The mass of one mole of a substance is called the molar mass or molecular weight. Examples: What is the molar mass of the following compounds? MgCl2 24.31 + 2(35.45) = 95.21 g/mol Mg(NO3)2 24.31 + 2(14.01) + 6(16.00) = 148.33 g/mol NaNO3 23.00 + 14.01 + 3(16.00) = 85.01 g/mol AgCl 107.9 + 35.45 = 143.4 g/mol (Note: Yes! You DO have to count significant figures when calculating molecular weight/molar mass. However, the number of significant figures may vary depending on which periodic table you use.) Chemists are generally interested in number of moles. Unfortunately, it is impossible to measure moles directly. However, masses are easily measured, and if the chemical formula of the compound is known, the molar mass can be used to determine the number of moles. The molar mass is defined as: molar mass = grams/moles = g/mol (1) Moles may be calculated by using molar mass as a conversion factor in dimensional analysis where molar mass in grams = 1 (exactly) mole of compound (2) This method is used in multi-step calculations. For example, if 0.873 g of MgCl2 is weighed out, it is 9.17 x 10-3 moles. 1 mole -3 0.873g x 95.21 g = 9.17 x 10 mol MgCl2 (3) However, 0.873 g of AgCl is only 6.09 x 10-3 mol. 1 mole 0.873g x 143.4 g = 6.09 x 10-3 mol AgCl (4) Molar mass may also be used to relate moles to grams. For example, 0.158 mol of MgCl2 is 15.2 g. 0.158 mol x 95.21 g = 15.2 g MgCl2 (5) 1 mol Percent is used to express parts per one hundred. Usually in chemistry, it refers to g of species of interest x 100 = % (6) g of whole thing Example: For the % Mg in MgCl2: In one mole of MgCl2, there are 24.31 g of Mg (molar mass of Mg, the part we are interested in) and 95.21 g of MgCl2 (the whole thing), so %Mg in MgCl2 is (24.31/95.21) x 100 = 25.53% Mg (7) PROCEDURE Work individually. The formula for calcium phosphate is Ca3(PO4)2. Weigh about 2 g of calcium phosphate to the nearest 0.001 g. In other words, you do not have to have exactly 2.000g, but you must know the weight you have exactly. Acceptable results include but are not limited to: 1.985g , 2.035g, 2.314g etc. Be sure to report all results with the correct number of significant figures and appropriate units! SYMBOLS, FORMULAS, MOLAR MASSES NAME__________________________ LABORATORY REPORT DATE__________________________ Part I. Symbols and Formulas In one mole of calcium phosphate, how many moles of each element are there? ______mol Ca _____ mol P _____ mol O Part II. Molar masses SHOW ALL CALCULATIONS. Mass of calcium phosphate sample plus weighing paper _______________________ Mass of weighing paper _______________________ Mass of calcium phosphate sample _______________________ Molar mass of calcium phosphate _______________________ Number of moles of calcium phosphate in your sample _______________________ Moles of phosphorus in your sample _______________________ Mass of phosphorus in your sample _______________________ Percent phosphorus in your sample _______________________ Percent of phosphorous in one mole of calcium phosphate _______________________ Questions Part I. 1. How many atoms of each element are present in one molecule of the compound? a. KNO3 b. (NH4)2SO4 2. How many moles of each element are present in two moles of the compound? a. CH3COOH b. Al(NO3)3 3. Write the appropriate chemical formulas for compounds with the following ratios of elements. a. 1 mole calcium: 1 mole carbon: 3 moles oxygen b. 1 molecule iron: 3 molecules chlorine c. 1 mole copper: 1 mole sulfur: 4 moles oxygen Part II. 4. What is the molar mass of each of the following compounds? Show all work. a. Ru(NH3)6Cl3 b. WO2 c. PbI2 5. What is the percent of the element which is underlined for each of the following compounds? Show all work. a. NaOH b. Al(NO3)3 6. Calculate the number of moles in the following samples. Show all work. a. 0.869 g of WO2 b. 2.200 g of PbI2 7. Calculate the number of grams in the following samples. Show all work. a. 0.20 mol of WO2 b. 0.067 mol of Ru(NH3)6Cl3 8. How is the %P in your sample of calcium phosphate related to the %P in one mole of calcium phosphate? Would you expect that relationship to always be true? Why or why not? .